Which one of the following statements best describes the following equilibrium at 298 K: CUCN(s) + CI (aq) = CuCl(s) + CN (aq) K = 2.0x10-13 at 298 K O The reaction is very reactant-favoured, and the cyanide concentration will be much smaller than the chloride concentration. O The reaction will proceed to the left until either CuCl or cyanide is fully consumed. O The reaction will proceed to the right until either CUCN or chloride is fully consumed. The direction and extent of reaction cannot be determined conclusively without knowing the sign and magnitude of the enthalpy change for the reaction, A-H. O The reaction is very product-favoured, and the chloride concentration will be much smaller than the cyanide concentration.

Which one of the following statements best describes the following equilibrium at 298 K: CUCN(s) + CI (aq) = CuCl(s) + CN (aq) K = 2.0x10-13 at 298 K O The reaction is very reactant-favoured, and the cyanide concentration will be much smaller than the chloride concentration. O The reaction will proceed to the left until either CuCl or cyanide is fully consumed. O The reaction will proceed to the right until either CUCN or chloride is fully consumed. The direction and extent of reaction cannot be determined conclusively without knowing the sign and magnitude of the enthalpy change for the reaction, A-H. O The reaction is very product-favoured, and the chloride concentration will be much smaller than the cyanide concentration.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Three reactions have the following K values: Reaction 1: K = 1.0 x 1015 Reaction 2: K = 7.1 x 10-5 Reaction 3: K = 1.5 x 10-16 Which equilibrium most favours the substances on the right side of the equation? And why?
A 0.066 mol sample of formaldehyde vapor, CH₂O, was placed in a heated 500 mL vessel and some of it decomposed. The reaction is CH,O(g) = At equilibrium, the CH₂O(g) concentration was 0.060 mol L-¹. Calculate the value of Kc for this reaction? Kc = H₂(g) H2(g) + CO(g) i
At 25°C, the equilibrium constant for the reaction Blg) + Clg) 2A(3) is K,-0.0735.If the three gases are mixed in a rigid container having partial pressuros of 3.35, 185 and 0.693 atm for A, B and C, respectively, is the system at equilibrium? The system is at equilibrium. The reverse reaction must proceed to establish equilibrium. The volume of the container must be known to answer the question. The concentrations of all substances must be known to answer the question. The forward reaction must praceed to establish equilibrium,
(5b) Write the expression for the equilibrium constant Kp for the following reaction.Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PNH3 )2 as (P NH3)2. If either the numerator or denominator is 1, please enter 1 2 CuCl2(s) ↔ 2 CuCl(s) + Cl2(g) K = (8c) Consider the following reaction where Kc = 6.50×10-3 at 298 K: 2 NOBr (g) 2 NO (g) + Br2 (g) A reaction mixture was found to contain 9.96×10-2 moles of NOBr (g), 4.61×10-2 moles of NO (g), and 4.42×10-2 moles of Br2 (g), in a 1.00 liter container.Indicate True (T) or False (F) for each of the following: 1. In order to reach equilibrium NOBr(g) must be consumed .2. In order to reach equilibrium Kc must decrease .3. In order to reach equilibrium NO must be produced .4. Qc is less than Kc.5. The reaction is at equilibrium. No further reaction will occur.
Cl3] ² [Hz] ² [A] [AC] Consider the chemical equation and equilibrium constant for the synthesis of ammonia at 25 °C: N₂ (g) + 3 H₂ (g) = 2 NH3 (g) K = 5.6 x 105 Calculate the equilibrium constant for the following reaction at 25 °C: NH3 (g) 1/2 N₂ (g) + 3/2 H₂ (g) K' = ? Kc = [NH3 ]² [₂] [H₂]] Kc- [~₂] ¹/2 [H NH3
Given the reaction: CO(NH2),(s) + H2O(g) = CO2(9) + 2NH3(g) -- Kp If this reaction system is initially at equilibrium and a catalyst is added, the new position of equilibrium will be = 1.39 at 500 K The value of K, for the given reaction at 600 K is The reaction CO(NH₂)₂(s) + H₂O(g) → CO₂(g) + 2 NH₂(g) is -- A flask containing CO₂(g), NH₂(g), CO(NH₂)₂(s) and H₂O(g) is initially at equilibrium at 500 K. When the flask is heated to 600 K, the amounts of CO(NH₂)₂(s) and H₂O(g) decrease and the amounts of CO₂(g) and NH₂(g) increase. This means that:
The equilibrium constant Kp = (9.180x10^-1) for the following reaction in the gas phase at a given temperature T: H2O(g) + Cl2O(g) = 2 HOCI(g) Calculate the equilibrium pressure (in bar) of HOCI(g) in the reaction vessel at temperature T if the initial pressures of H2O(g) and Cl₂O(g) are both equal to (3.06x10^-1) bar.
At room temperature when HI (aq) is added to potassium bisulfite, KHSO3(s), sulfur dioxide is formed and the reaction vessel becomes cold. HI (aq) + KHSO3(s)→ SO2(g) + H2O(l) + K+(aq) + I-(aq). A.)Once the process has reached equilibrium at room temperature, which of the following must be true? choose one....(ΔH<TΔS, ΔH=TΔS, ΔH>TΔS, or need more info). B.) Once the process has reached equilibrium at room temperature, which of the following must be true? choose one....(ΔSuniv<0, ΔSuniv=0, ΔSuniv>0, or need more info).
The equilibrium constant, Kp, for the following reaction is 0.215 at 673 K. Calculate K. for this reaction at this temperature. NH4I(s) =NH3(g) + HI(g) Kc
write your answer in scientific notation
Consider the reaction: CH3COOH (aq) + H₂O(1) K = 1.8 x 10-5 at 25 °C Part A If a solution initially contains 0.225 mol L-¹ CH3COOH, what is the equilibrium concentration of H3O+ at 25 °C? Express your answer in moles per litre to two significant figures. 15. ΑΣΦ [H3O+] = H3O+(aq) + CH3COO (aq) Submit Request Answer ? mol L-1
3 A + 2B 1 C Calculate the equilibrium constant (K) for the following reaction at 1000. K, using this information: A and B are placed in a flask and at the beginning of the reaction [A] is 6.87 M and [B] is 6.38 M. After the reaction has reached equilibrium, [C] is 1.47 M. Unfortunately, significant figures cannot be taken into account here, so please ignore them this time. 119.84085 0.00132 0.00011 0.03354 0.00834 1 1 1